Question

According to VBT, any covalent bond will be formed by overlapping of atomic orbitals of bonded atoms provided atomic orbitals must be half-filled and electrons be in opposite spin.
According to type of overlapping, covalent bonds can be classified as:
(a) $\sigma$ bond
(b) $\pi$ bond
(c) $\delta$ bond
Which of the following set of orbitals does not produce nodal plane in $xz$ - plane:

• A. None of the these
• B. $d_{xy}+d_{xy}$
• C. $p_y+d_{xy}$
• D. $d_{yz}+d_{yz}$

Answer 1

The correct option is A None of the these

For option (a):
Type of orbital combination: $d_{yz}+d_{yz}$
For $\pi$ bond:
Internuclear axis: $y$-axis and $z$-axis
Nodal plane: $xy+xz$
For $\sigma$ bond:
axis: $x$-axis
Nodal plane: $xy$ and $xz$

For option (b):
Type of orbital combination: $d_{xy}+d_{xy}$
For $\pi$ bond:
Internuclear axis: $x$-axis and $y$-axis
Nodal plane: $xz+yz$
For $\sigma$ bond:
axis: $z$-axis
Nodal plane: $xz$ and $yz$

For option (c):
Type of orbital combination: $p_y+d_{xy}$
For $\pi$ bond:
Internuclear axis: $x$-axis
Nodal plane: $xz$
No $\delta$ bond formation
Therefore, option (d) is correct.